WCH12 01 2024 Jan QP
WCH12 01 2024 Jan QP
WCH12 01 2024 Jan QP
com
Please check the examination details below before entering your candidate information
Candidate surname Other names
Instructions
• Use black ink or ball-point pen.
• IfFillpencil is used for diagrams/sketches/graphs it must be dark (HB or B).
• centrein the boxes at the top of this page with your name,
number and candidate number.
• Answer all questions.
• Answer the questions in the spaces provided
– there may be more space than you need.
• Show all your working in calculations and include units where appropriate.
Information
• The total mark for this paper is 80.
• The marks for each question are shown in brackets
– use this as a guide as to how much time to spend on each question.
• structure
In the question marked with an asterisk (*), marks will be awarded for your ability to
your answer logically, showing how the points that you make are related or
follow on from each other where appropriate.
• There is a Periodic Table on the back cover of this paper.
Advice
• Read each question carefully before you start to answer it.
• Try to answer every question.
• Check your answers if you have time at the end. Turn over
P75592A
©2024 Pearson Education Ltd.
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SECTION A
Answer ALL the questions in this section.
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You should aim to spend no more than 20 minutes on this section.
For each question, select one answer from A to D and put a cross in the box . If you change
your mind, put a line through the box and then mark your new answer with a cross .
A HF
B H2Te
C AsH3
D SnH4
(Total for Question 1 = 1 mark)
A H2(g) → 2H(g)
B H2O(l) → H2O(g)
C H2(l) → H2(g)
3 A compound contains
• molecules with non-polar bonds
• permanent dipole-permanent dipole forces between its molecules.
What could be the formula of this compound?
Use the Data Booklet as a source of information.
A NO
B BeCl2
C PH3
D CI4
(Total for Question 3 = 1 mark)
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4 Which alkane has the strongest London forces in the liquid phase?
A (CH3)4C
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B CH3CH2CH2CH2CH3
C (C2H5)4C
D CH3(CH2)7CH3
(Total for Question 4 = 1 mark)
5 In which liquid solvent would the solubility of lithium chloride (LiCl) be lowest?
A ammonia
B cyclohexane
C methanol
D water
(Total for Question 5 = 1 mark)
6 Which compound does not contain an element with an oxidation number of –1?
A HF
B NaH
C H2O2
D CH4
(Total for Question 6 = 1 mark)
A Br2 + F2 → 2BrF
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A BaCl2 and AgNO3
A sodium carbonate
B sodium hydroxide
C nitric acid
D ammonia
(Total for Question 9 = 1 mark)
What is the minimum volume, in cm3, of 0.5 mol dm–3 Na2S2O3(aq) needed to react
completely with 0.01 mol of Br2(l)?
A 0.01
B 0.04
C 10
D 40
(Total for Question 10 = 1 mark)
Use this space for any rough working. Anything you write in this space will gain no credit.
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11 What is the mass of nitrogen atoms in 50 cm3 of a 2.0 mol dm–3 solution of
ammonium nitrate, NH4NO3(aq)?
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A 35 g
B 8.0 g
C 2.8 g
D 1.4 g
(Total for Question 11 = 1 mark)
12 Which row shows the correct trends down the group for the elements of Group 7?
Reactivity as
Boiling temperature Electronegativity
oxidising agent
A increases decreases decreases
13 Which statement best explains why the rate of a chemical reaction increases with
increasing temperature?
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by pressure and by catalysts
B the concentration of reactants is constant
A 1-bromobutane
B 1-chlorobutane
C 1-fluorobutane
D 1-iodobutane
(Total for Question 15 = 1 mark)
16 What is the total number of structural isomers for cyclic alcohols with the molecular
formula C4H8O?
A 2
B 3
C 4
D 5
(Total for Question 16 = 1 mark)
Use this space for any rough working. Anything you write in this space will gain no credit.
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A 1, 2 and 3
B 1 and 3 only
C 2 and 3 only
D 1 only
(Total for Question 18 = 1 mark)
OH OH O OH
HO OH O O
A 2
B 3
C 4
D 5
(Total for Question 19 = 1 mark)
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100
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80
60
Relative
intensity
40
20
0
10 15 20 25 30 35 40 45 50 55 60
m/z
A CH3COOH
B CH3COCH3
C CH3CH2CHO
D CH3CH2CH2CH3
(Total for Question 20 = 1 mark)
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SECTION B
Answer ALL the questions. Write your answers in the spaces provided.
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21 This question is about the element calcium and some of its compounds.
(a) Give the complete electronic configuration, using s, p, d notation, of a
calcium atom in the ground state.
(1)
(ii) Complete the table to indicate the type(s) of bonding and structure in the
species involved in this reaction.
(3)
Ca(s)
covalent
giant
(iii) State the expected flame colour when CaCl2 is used in a flame test.
(1)
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(c) A sample of solid anhydrous calcium nitrate, Ca(NO3)2(s), is heated strongly for
several minutes in the apparatus shown.
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Ca(NO3)2(s)
water containing
heat universal indicator
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(ii) Explain why the observations from (c)(i) would be made more quickly if
the experiment was repeated with solid anhydrous magnesium nitrate,
Mg(NO3)2(s).
(3)
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*(d) Samples of calcium and magnesium are added to separate test tubes of
cold water containing a few drops of universal indicator.
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State and explain the differences in the observations made in each experiment.
Include an equation in your answer.
(6)
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in kJ mol–1, for Reaction 1.
Reaction 1 Mg(s) + ½O2(g) → MgO(s) ΔrH1
(a) Explain why ΔrH1 can also be described as an enthalpy change of formation.
(2)
(b) The student carried out an experiment to determine the enthalpy change of
reaction, ΔrH2 , in kJ mol–1, for Reaction 2.
Reaction 2 MgO(s) + 2HCl(aq) → MgCl2(aq) + H2O(l) ΔrH2
0.189 g of solid magnesium oxide was added to excess hydrochloric acid in a
polystyrene cup and stirred until the reaction was complete.
The total mass of the solution formed was 25.0 g.
During the experiment, the temperature increased from 21.5°C to 28.0°C.
Calculate ΔrH2 , in kJ mol–1, including a sign.
Give your answer to an appropriate number of significant figures.
[ Specific heat capacity of the solution = 4.18 J g–1 °C–1. ]
(4)
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[If you did not calculate an answer to (b), use a value of –100 kJ mol–1.
This is not the correct answer.]
(2)
Data
Mg(s) + 2HCl(aq) → MgCl2(aq) + H2(g) ΔrH = –462 kJ mol–1
H2(g) + ½O2(g) → H2O(l) ΔfH = –286 kJ mol–1
Enthalpy cycle
ΔrH1
Mg(s) + ½O2(g) MgO(s)
2HCl 2HCl
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(1)
(ii) Draw the displayed formula of the only C4H9Br secondary bromoalkane.
(1)
(b) Give the structure of the C4H9Br bromoalkane that would react fastest with
aqueous silver nitrate in ethanol.
(1)
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CH3CH2CH2CH2OH
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R1
R4 R2
CH3CH2CH2CH2CN CH3CH2CH2CH2Br CH3CH2CH CH2
R3
CH3CH2CH2CH2NH2
Formula
Reaction Name of mechanism of Condition(s)
reagent
R1 nucleophilic substitution
R2 heat in ethanol
R3 NH3
R4 heat in ethanol
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NH3
H H H
H H H
NH3
CH3CH2CH2CH2NH2 + NH4+
(iii) Give the wavenumber range of an absorption in the infrared spectrum of the
organic product of reaction R4, which is not present in the infrared spectrum
of CH3CH2CH2CH2Br.
Indicate the bond responsible for this absorption.
(2)
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SECTION C
Answer ALL the questions. Write your answers in the spaces provided.
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24 The elements of Group 7, the halogens, have many important uses.
Fluorine is used to make sulfur hexafluoride, SF6 , a gas which is used
as an insulator in electrical equipment.
Chlorine is used as a bleach and as a disinfectant in water treatment.
Bromine is used to make organic chemicals that are used as fire retardants.
Iodine has been used in the catalyst in the manufacture of ethanoic acid.
(a) SF6 can be made from the reaction of sulfur, S8 , with fluorine.
S S
S S
S S
S S
S S 268
F F 151
(i) Calculate the mean bond enthalpy, in kJ mol–1, for a single S F bond.
(3)
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(ii) Give two reasons why your answer to (a)(i) is unlikely to accurately represent
the true S F bond enthalpy in SF6 .
(2)
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Cl2(g) + 2NaOH(aq) → NaClO(aq) + NaCl(aq) + H2O(l)
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Br
Br Br
Br
Br
Br
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(d) The industrial manufacture of ethanoic acid first used an iodine-based catalyst.
Explain, with the aid of a labelled Maxwell–Boltzmann distribution, how a catalyst
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increases the rate of a chemical reaction.
(4)
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